How many milliliters of .50 M NaOH solution are required to titrate 40.0 mL of a 0.10 M H2SO4 solution to an end joint?
2NaOH + H2SO4 ---> Na2SO4 + 2H2O
n = (Molarity)(vol)
n= (0.10M)(0.04L)
=0.004moles of H2SO4
0.004molesH2SO4 * 2moles NaOH/1mole H2SO4
= 0.008moles NaOH
so M= n/v
v=n/M
= 0.008/0.50
= 0.004L
0.004*1000
= 4.0 ml
Correction to response by Zoe
2NaOH + H2SO4 ---> Na2SO4 + 2H2O
n = (Molarity)(vol)
n= (0.10M)(0.04L)
=0.004moles of H2SO4
0.004molesH2SO4 * 2moles NaOH/1mole H2SO4
= 0.008moles NaOH
so M= n/v
v=n/M
= 0.008/0.50
OK to here.
0.008 moles/0.50 L = 0.016 L or 16 mL.
= 0.004L
0.004*1000
= 4.0 ml
To determine the volume of a 0.50 M NaOH solution required to titrate 40.0 mL of a 0.10 M H2SO4 solution, you need to use the balanced chemical equation for the reaction between NaOH and H2SO4:
2 NaOH + H2SO4 -> Na2SO4 + 2 H2O
From the balanced equation, you can see that the ratio of NaOH to H2SO4 is 2:1. This means that to neutralize one mole of H2SO4, you'll need two moles of NaOH.
First, calculate the number of moles of H2SO4 in the 40.0 mL of 0.10 M H2SO4 solution using the formula:
moles = concentration (M) × volume (L)
moles of H2SO4 = 0.10 mol/L × 0.040 L = 0.004 mol
Since the ratio between H2SO4 and NaOH is 1:2, you'll need twice as many moles of NaOH to neutralize the H2SO4. Therefore, you need 0.004 mol × 2 = 0.008 mol of NaOH.
Now, you need to use the concentration of the NaOH solution to calculate the volume of NaOH required:
moles = concentration (M) × volume (L)
0.008 mol = 0.50 mol/L × volume (L)
volume (L) = 0.008 mol ÷ 0.50 mol/L = 0.016 L
Finally, convert the volume to milliliters:
Volume (mL) = 0.016 L × 1000 mL/L = 16 mL
Therefore, you would need 16 milliliters of the 0.50 M NaOH solution to titrate 40.0 mL of the 0.10 M H2SO4 solution to the end point.
To find the number of milliliters of 0.50 M NaOH solution required to titrate 40.0 mL of 0.10 M H2SO4 solution, we can use the concept of stoichiometry.
The balanced chemical equation for the reaction between NaOH and H2SO4 is:
2 NaOH + H2SO4 -> Na2SO4 + 2 H2O
From the balanced equation, we can see that it takes 2 moles of NaOH to react with 1 mole of H2SO4.
First, let's calculate the number of moles of H2SO4 in the 40.0 mL solution:
moles of H2SO4 = volume (in liters) × concentration (in M)
= 0.040 L × 0.10 mol/L
= 0.004 mol
According to the stoichiometry of the reaction, it takes 2 moles of NaOH to react with 1 mole of H2SO4. Therefore, we need double the number of moles of NaOH compared to H2SO4.
moles of NaOH = 2 × moles of H2SO4
= 2 × 0.004 mol
= 0.008 mol
Now, let's calculate the volume of 0.50 M NaOH solution needed to provide 0.008 moles of NaOH:
volume of NaOH solution (in liters) = moles of NaOH / concentration (in M)
= 0.008 mol / 0.50 mol/L
= 0.016 L
Since the concentration is given in moles per liter, we have calculated the volume in liters. To convert it to milliliters, we multiply it by 1000:
volume of NaOH solution (in milliliters) = 0.016 L × 1000
= 16 mL
Therefore, 16 milliliters of 0.50 M NaOH solution are required to titrate 40.0 mL of 0.10 M H2SO4 solution to an end point.